A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200 . g of water (see sketch at right). First, a 7.000g tablet of benzoic acid (C6H5CO2H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454kJ/g.) The temperature of the water is observed to rise from 25.00C to 57.15C over a time of 9.1 minutes. Next, 5.340g of acetaldehyde (C2H4O) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 25.00C to 50.34C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: 2C2H4O(g)+5O2(g)4CO2(g)+4H2O(g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction